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CHEM 23: Stoichiometric Calculations: The Workhorse of the Analyst

front 1

stoichiometry

back 1

the ratios in which chemicals react, from which we apply appropriate conversion factors to arrive at the desired calculated results

front 2

definition of avogadro's number

back 2

tells the number of particles in 1 mole (or mol) of a substance.

front 3

avogadro's number

back 3

6.022x1023

front 4

atomic weight

back 4

is the weight of a specified no. of atoms in that element

front 5

molecular weight

back 5

the sum of the atomic weights of the atoms that make up a compound

front 6

Find the molecular weight of HCl

back 6

(1.0080)+(35.45) = 36.458 g/mol (insert surname)

front 7

formula weight

back 7

sum of atomic weights but for ionic compounds

front 8

Find the formula weight of NaOH

back 8

(22.990) + (12.011) + (1.0080) = 40 g/mol (insert surname)

front 9

equivalent weight

back 9

the mass of one equivalent, that is the mass of a given substance which will combine with or displace a fixed quantity of another substance

front 10

formula of equivalent weight

back 10

front 11

percent by mass

back 11

is the ratio of the mass of a solute to the mass of the solution multiplied by 100 percent

front 12

formula of percent by mass

back 12

front 13

A sample of 0.894 grams (g) of potassium chloride (KCl) is dissolved in 54.8 grams of water. What is the percent by mass of KCl in the solution?

back 13

1.61%

front 14

percent by volume

back 14

a unit of concentration used to express the amount of solute in a solution as a percentage of the volume of the solution.

front 15

formula of percent by volume

back 15

front 16

In a solution, there is 122.4 mL solvent and 5.24 ml solute present. Find the percent by volume.

back 16

4.11%

front 17

mole

back 17

amount or sample of a chemical substance that contains as many constitutive particles as there are atoms in 12 grams = carbon – 12 (12g C-12 = 1mol)

front 18

formula of mole

back 18

front 19

molarity

back 19

one-molar solution is defined as one that contains one mole of substance in each liter of solution

front 20

formula of molarity

back 20

front 21

normality

back 21

one normal solution contains one equivalent per liter

front 22

formula of normality

back 22

front 23

dilution

back 23

for preparation of a smaller concentration

front 24

formula of dilution

back 24

C1V1=C2V2

front 25

parts per million

back 25

represents the number of parts of a substance per million parts of the solution

front 26

formula of parts per million

back 26

front 27

A solution has a concentration of 1.24 g/L. What is its concentration in ppm?

back 27

1240 ppm